At 1500^$\circ$C the equilibrium constant for the reaction CO(g) + 2H₂(g) $\leftrightharpoons$ CH₃OH(g) has the value K_p = 1.4 * 10^-7. Calculate $\Delta$G^$\circ$ for this reaction at 1500^$\circ$C. A) 105 kJ/mol B) 1.07 kJ/mol C) -233 kJ/mol D) -105 kJ/mol E) 233 kJ/mol

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The Answer of At 1500^$\circ$C the equilibrium constant for the reaction CO(g) + 2H₂(g) $\leftrightharpoons$ CH₃OH(g) has the value K_p = 1.4 * 10^-7. Calculate $\Delta$G^$\circ$ for this reaction at 1500^$\circ$C. A) 105 kJ/mol B) 1.07 kJ/mol C) -233 kJ/mol D) -105 kJ/mol E) 233 kJ/mol

At 1500 ∘\circ∘ C the Equilibrium Constant for the Reaction CO(g) + 2H2(g)

At 1500^$\circ$C the Equilibrium Constant for the Reaction CO(g) + 2H₂(g)